THURSDAY, DECEMBER 3 RD Grab your poster You have 10 minutes to finish it When you’re done, hang it on the board and grab notes off the projector.

Slides:



Advertisements
Similar presentations
Solubility Equilibria
Advertisements

Solubility Equilibria
Equilibrium 1994A Teddy Ku A MgF 2(s) Mg 2+ (aq) + 2F - (aq) In a saturated solution of MgF 2 at 18 degrees Celsius, the concentration of Mg 2+
Solubility (Precipitation Equilibria: The solubiloity Product- Section 10.5 (p ) Chapter 10.
Solubility Equilibria AP Chemistry
Chapter 19 - Neutralization
AQUEOUS EQUILIBRIA AP Chapter 17.
What’s solutions? Electrolytes SolubilityReactionsRandy $100 $200 $300 $400 $500.
Solubility Equilibrium
CHEMISTRY 121/122 Solubility Equilibrium. What is a solution?  A solution is a mixture in which a solid has been dissolved into a liquid, usually water.
Aqueous Equilibria Entry Task: Feb 28 th Thursday Question: Provide the K sp expression for calcium phosphate, K sp = 2.0 x From this expression,
Acid-Base Equilibria and Solubility Equilibria Chapter
Solubility. Solubility “Insoluble” salts are governed by equilibrium reactions, and are really sparingly soluble. There is a dynamic equilibrium between.
Solubility. Solubility “Insoluble” salts are governed by equilibrium reactions, and are really sparingly soluble. There is a dynamic equilibrium between.
The K sp of chromium (III) iodate in water is 5.0 x Estimate the molar solubility of the compound. Cr(IO 3 ) 3 (s)  Cr 3+ (aq) + 3 IO 3 - (aq)
Lecture 72/1/06. Precipitation reactions What are they? Solubility?
Chapter 16: Aqueous Ionic Equilibria Common Ion Effect Buffer Solutions Titrations Solubility Precipitation Complex Ion Equilibria.
Review of Solubility and Precipitation Reactions
Solubility Product Constant
Unless otherwise stated, all images in this file have been reproduced from: Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 2007 (John Wiley)
1 Solubility Equilibria all ionic compounds dissolve in water to some degree –however, many compounds have such low solubility in water that we classify.
CHM 112 Summer 2007 M. Prushan Acid-Base Equilibria and Solubility Equilibria Chapter 16.
Additional Aspects of Aqueous Equilibria BLB 11 th Chapter 17.
Prentice Hall © 2003Chapter 4 Chapter 4 Aqueous Reactions and Solution Stoichiometry CHEMISTRY The Central Science 9th Edition David P. White.
Chapter 16 Aqueous Ionic Equilibria. Common Ion Effect ● Water dissolves many substances and often many of these interact with each other. ● A weak acid,
Solubility Equilibrium
Friday, March 21 st : “A” Day Monday, March 24 th : “B” Day Agenda  Homework questions/collect  Finish section 14.2: “Systems At Equilibrium”  Homework:
Unit 7 - Chpt 16 - Solubility equilibria and Quantitative analysis Solubility equilibria and Ksp Predict precipitation Qualitative analysis HW set1: Chpt.
Chapter 16 Lesson 1 Solubility and Complex Ion Equilibria.
PRECIPITATION REACTIONS
Solubility Equilibria
Dressen.  Understand the dynamics of a dissolving substance.  Be able to construct a K sp equlibrium expression (solubility product constant).  Be.
Aqueous Equilibria Entry Task: Feb 17 th Wednesday Notes on Precipitate and ions HW: Precipitate and ions ws MAYHAN.
Prentice Hall © 2003Chapter 4 Chapter 4 Aqueous Reactions and Solution Stoichiometry.
Chapter 15 Applications of Aqueous Equilibria. The Common Ion Effect A common ion is an ion that is produced by multiple species in solution (other than.
Solubility Chapter 17. No only do acids and bases dissolve in aqueous solutions but so do ionic compounds –Many ionic compounds tend to be strong electrolytes.
Terms Solute Substance that has been dissolved in a liquid Solvent the solution (liquid or gas) part of the solute concentration Dissolves the solute Solubility.
Chapter 9 Chemical Equilibrium
Chapter 21 Notes, part III Ksp and Common Ion Effect.
1 Titration Curve of a Weak Base with a Strong Acid.
Hannah Nirav Joe ↔. Big Ideas You will be able to Understand what K sp is Find K sp from a reaction.
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Solubility Equilibrium Chapter 7. The Solubility Equilibrium Remember from SPH3U: Solubility is the amount of solute that dissolves in a given amount.
Unit 17. Dissolution: the process in which an ionic solid dissolves in a polar liquid. AgCl (s) ↔ Ag + (aq) + Cl - (aq) Precipitation: the process in.
K sp = [M x+ ] [N x– ] Solubility Equilibria -- involve the dissolution or precipitation of “insoluble” salts Consider a saturated solution of a typical.
K sp solubility product constant shows dissolution of “insoluble” ionic salts MgF 2(s) Ca 3 (PO 4 ) 2 K sp values in Ch. 16 and Appendix II of textbook.
Saturated solution – no more solute will dissolve solubility product constant – equilibrium constant for ionic compounds that are only slightly soluble.
Additional Aspects of Aqueous Equilibria Chapter 17.
Solubility & SOLUBILITY PRODUCT CONSTANTS. Solubility Rules All Group 1 (alkali metals) and NH 4 + compounds are water soluble. All nitrate, acetate,
Solubility Equilibria 16.6 AgCl (s) Ag + (aq) + Cl - (aq) K sp = [Ag + ][Cl - ]K sp is the solubility product constant MgF 2 (s) Mg 2+ (aq) + 2F - (aq)
Solubility Equilibrium Solubility Product Constant Ionic compounds (salts) differ in their solubilities Most “insoluble” salts will actually dissolve.
Solubility Equilibria
To calculate the new pH, use the Henderson- Hasselbalch equation: 1141.
Chem. 1B – 10/8 Lecture. Announcements I Lab –Quiz 5 next Monday and Tuesday – Topics: titrations, solubility and experiments 3 and 4 –Experiment 4 –
Tuesday, December 1 st  Grab a notes sheet off the projector  Please take out the following:  Purple sheet  Review questions  Yesterday’s worksheet.
Chapter 16: Aqueous Ionic Equilibria CHE 124: General Chemistry II Dr. Jerome Williams, Ph.D. Saint Leo University.
Monday, November 9 th Grab a blue sheet from on top of the projector. Take out: packet -Review questions notes Write the chemical.
BUFFERS SUROVIEC SPRING 2014 Chapter I. Buffer Solutions A. Buffer is a solution that resists a change in pH with the addition of small amounts.
CHE1102, Chapter 17 Learn, 1 Chapter 17 Solubility and Simultaneous Equilibria.
Acid-Base Equilibria and Solubility Equilibria Chapter 16 Semester 2/2014 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction.
Solubility Equilibria.  Write a balanced chemical equation to represent equilibrium in a saturated solution.  Write a solubility product expression.
Aqueous SolutionsAqueous Solutions  Compounds dissolved into water.  Can contain molecules or ions in a solution.  How do you distinguish between ion.
Solubility Equilibria Will it all dissolve, and if not, how much will?
Chem. 1B – 10/6 Lecture.
Solubility Equilibria Review Section 17.4
17.4: Solubility Equilibria
Chem. 1B – 10/4 Lecture.
Chapter 13 Reaction Rates and Chemical Equilibrium
Kc Ksp!!!!! Kp Kw Ka Kb.
Solubility Product KSP.
Presentation transcript:

THURSDAY, DECEMBER 3 RD Grab your poster You have 10 minutes to finish it When you’re done, hang it on the board and grab notes off the projector

SOLUBILITY The equilibrium constant for the dissociation of a solid salt into its aqueous ions is called the solubility product, K sp. For an ionic solid M n X m, the dissociation reaction is M n X m (s)  nM m+ (aq) + mX n− (aq). The solubility product would be K sp = [M m+ ] n [X n− ] m. For example, the dissociation reaction for PbCl 2 is PbCl 2 (s)  Pb 2+ (aq) + 2 Cl − (aq). And its equilibrium constant is K sp = [Pb 2+ ][Cl − ] 2.

MOLAR SOLUBILITY Solubility is the amount of solute that will dissolve in a given amount of solution at a particular temperature. The molar solubility is the number of moles of solute that will dissolve in a liter of solution. The molarity of the dissolved solute in a saturated solution For the general reaction M n X m (s)  nM m+ (aq) + mX n− (aq)

K SP AND RELATIVE SOLUBILITY Molar solubility is related to K sp. But you cannot always compare solubilities of compounds by comparing their K sp s. To compare K sp s, the compounds must have the same dissociation stoichiometry.

K SP AND COMMON IONS Just like with any other equilibrium, ions in common will drive the reaction backwards In the case of solubility, it will lead to precipitation pH and Ksp Consider the insoluble compound MgF 2 If you put it in a low pH (high hydrogen ion concentration) solution, some of those F- ions will bond with hydrogen to form the weak acid HF Thus, low pH solutions increase the solubility of compounds that contain anions of weak acids

Friday, 12/4 Quiz on Due: Review questions and problem set 5 Monday, 12/7 Ch 17 review and practice Due: Chapter 5 packet and problem set 6 (cumulative questions, to be handed out tomorrow) and quiz corrections Tuesday, 12/8 Chapter 17 review and practice Last day I’ll check ch 17 HW Wednesday, 12/9 Chapter 17 exam Thursday, 12/10 Titration lab Chapter 16 retake deadline Friday, 12/11 Chapter 5 review day Monday, 12/14 Chapter 5 test Tuesday, 12/15-Friday, 12/18 Begin chapter 19 ANNOUNCEMENTS